Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

General Chemistry 111 > Chapter 9 > Flashcards

Chapter 9 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

what is a chemical bond

A

a strong attractive force that exists between neighboring atoms in a substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

three types of chemical bonds

A
  • ionic
  • covalent
  • metallic
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is a metallic bond

A

a regular arrangement of metal atoms, but the valence electrons move throughout the crystal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is an ionic bond

A

a chemical bond formed by the electrostatic attraction between positive and negative ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

when do ionic bonds form

A

when one or more electrons are transferred from the valence shell of one atom to the valence shell of another atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

the atom that transfers electrons in ionic bonds

A

cation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

the atom that gains electrons in an ionic bond

A

anion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

G.N Lewis

A

introduced the Lewis Electron-Dot symbol to describe ions and molecules by considering a “cubical atom”

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

G.N Lewis and his hypothetical “cubical atom”

A

there is space for 8 electrons at the corners of a hypothetical cube

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what did G.N Lewis recognize about atoms

A

there is a “kernel” of electrons that remain uncharged, and an outer shell that varies during chemical reactions between 0 and 8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

valence electrons

A

the outer shell electrons of an atom. they are the electrons that participate in chemical bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Lewis’s Cubical Atom (definition)

A

a cube provides a simple means to illustrate valence electrons around an atom, but this is more commonly represented in 2-dimensions using “dots” to represent the valence electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Lewis dot symbol

A

a notion in which the electrons in the valence shell of an atom or ion are represented by dots placed around the chemical symbol of the element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

how are lewis dot symbols placed

A

dots are placed one to a side until all 4 sides are occupied

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what concept did Lewis introduce

A

the electron-pair bond and the “group of 8” electrons being the favorable situation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

what did Lewis’s concept lead to

A

-the octet rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

octet rule definition

A

-molecules or ions tend to be most stable when the outermost electron shells contain 8 electrons and have structures that are isoelectronic with the noble gasses

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what does the combination of ionization energy and electron affinity need

A

it needs energy because it is endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

lattice energy

A

the change in energy when an ionic solid is separated into gas-phase ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

what happens when 2 ions bond

A

energy is released, making the overall process exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

according to Coulombs law, what 2 factors affect the strength of the ionic bond

A
  • charge (Q)

- size of the ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Coulomb’s Law

A

the energy (E) obtained in bringing 2 ions with electric charges Q+ and Q- from infinite separation to a distance (r) apart

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

equation for coulomb’s law

A

E=(Q+ x Q-)/r

24
Q

Q+

A

the charge on the cation

25
Q

Q-

A

the charge on the anion

26
Q

r

A

the distance between the ions

27
Q

what does solving for E in coulomb’s law give you

A

the strength of the ionic bond

28
Q

ionic substances are typically ________ solids

A

high-melting

29
Q

what 2 factors affect the strength of the ionic bond (Melting point: Coulomb’s Law

A

melting point (strength of ionic bond) increases as Q increases and/or as r decreases

30
Q

covalent bond

A

a chemical bond formed by sharing a pair of electrons

31
Q

how do we understand how covalent bonds form

A
  • we monitor the energy of two isolated hydrogen atoms as they move closer together
  • the energy decreases, first gradually and then more steeply, to a minimum
  • as the atoms continue to move closer, energy starts to increase dramatically because the nuclei repel
32
Q

bond length

A

the distance between the atoms when energy is at a minimum

33
Q

what is the importance of the Born-Haber Cycle

A

because it is very difficult to measure the lattice energy directly, using the energy changes for steps helps make it easier and gives the same result

34
Q

Orbitals

A

a place to put electrons

35
Q

Elements to the left of carbon have __________ and those to the
right have ________

A

empty orbitals

filled orbitals (lone pairs)

36
Q

coordinate covalent bond

A

is one where a single atom provides

both electrons

37
Q

Bond Lengths sorted by size

A

Triple bond < Double Bond < Single Bond

38
Q

Ionization energy and electron affinity provide

A

an
indication of how readily an atom may want to give up or
accept an electron

39
Q

Electronegativity is considered to be

A

the ability of an atom

in a molecule to attract electrons to itself.

40
Q

Linus Pauling

A

quantified the concept of electronegativity by comparing the
bond energy of a heteronuclear A-B bond with the corresponding
homonuclear A-A and B-B bond energies.

41
Q

The bond energy E(A-B) for a molecule A-B is always

A

greater than

the mean of the bond energies

42
Q

Pauling argued that the excess bond energy is due to the

A

ionic

component caused by the partial charges on the atoms in AB.

43
Q

Electron Affinity versus Electronegativity

A

Electron Affinity: measurable, Cl is highest.

Electronegativity is the ability of an atom to attract toward
itself the electrons in a chemical bond.
Electronegativity: relative, F is highest

44
Q

when the difference in electronegativity is 0

A

the bond is covalent

45
Q

when the difference in electroegativity is greater than or equal to 2

A

the bond is ionic

46
Q

when the difference in electronegativity is between 0 and 2

A

the bond is polar covalent

47
Q

Formal charge results from assuming

A

equal sharing of the

bonding electrons

48
Q

The formal charge on an atom in a Lewis dot structure is

determined by inspecting

A

how many lone pairs are present and

how many bonds it forms.

49
Q

The sum of the formal charges of the atoms in a molecule or ion
must equal

A

the charge on the molecule or ion.

50
Q

Resonance

A

means that the actual structure is a composite or an

average of the two structures.

51
Q

classic example of “resonance”.

A

benzene

52
Q

A “circle” is used to depict the fact that

A

the bonding cannot be
properly represented by a single Lewis structure in which a
“line” represents a shared electron pair bond

53
Q

Exceptions to the Octet Rule

A
  1. The incomplete octet
    (hypovalent or electron deficient molecules).
  2. Odd-electron molecules
  3. Hypervalent molecules (“valence shell expansion”)
54
Q

Bond order

A

is the number of pairs of electrons in a bond.

55
Q

bond energy

A

The enthalpy change required to break a particular bond into one mole of
gaseous molecules

56
Q

Bond energy is a measure of

A

bond strength: the greater the bond energy,

the stronger the bond, the more stable the molecule

57
Q

Bond energies can be used to estimate the

A

enthalpy change, ΔH, for a

reaction

General Chemistry 111 (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions